(Polar molecules, Non-polar molecules, etc.)
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The bond angle is going to be slightly less than 109 because of the lone pair repulsion. Because there are 4 regions of electron density, the electron geometry would be tetrahedral and 109.5 bond angles, but for the molecular geometry you have to take the lone pairs into account.
Adding on to the reply above me, the lone pairs distort the attached atoms more than normal bonding pairs do because when they aren't engaged in a bond, electrons move more freely and this causes them to be more repulsive. Because of this, the lone pairs take up more room than atoms do and thus push the bonded atoms away and towards each other, resulting in their bond angles shrinking. Hope this helped!
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